Saturation of Salt-Solutions. 

 Table V. 



545 



Salts. 



E. 



Compound 

 molecules. 



A. 



B. 



AxB. 



(AxB) 



+ 1800. 



Mol. 



TOl. 



Diff. 



KC1 



NaCl 



NaCl 



NaN0 3 ... 



KNO3 ... 

 KC1 



KNO3 ... 



NaN0 3 ... 



1 



1-66 



1 

 1-444 



1 



2-36 



1 

 2-45 



4-795 



7-64 



3-42 



7*87 



30-9 

 21-2 



21-2 

 34-2 



41-4 

 309 



41*4 

 34-2 



4-795 



7-96 



7-64 

 1103 



342 



8-07 



7-87 

 19-29 



148-2 



168-8 



161-2 

 377-2 



141-6 

 249-4 



325-8 

 659-7 



21170 

 2338-5 

 2191-0 



2785-5 



2120-8 

 2339-1 

 2200-9 

 2830-6 



+3-8 

 +'6 

 +9-9 

 +45-1 



A = mean mol. vol. in saturated solution of the salt alone. 



B= number of salt-molecules present in the saturated solution of both salts. 



present in a saturated solution per 100 H 2 0. Comparing 

 these numbers with those in Table IV., we find that in 

 Case (1) the solubibity has increased for : — 



NaCl 

 KC1 



Case (2), 

 NaCl 

 NaN0 3 



Case (3), 

 KNO3 

 KC1 



Case (4), 

 KNO3 

 NaN0 3 



from 10-99 to 15-92 

 8-38 „ 9-59 







» 

 » 



10-99 

 18-45 



5-68 

 8-38 



5-68 

 18-45 



15-28 

 22-06 



6-84 

 16-14 



15-74 

 38-58 



This is on the assumption that each salt takes one half of the 

 water present in the solution. The solubility has therefore 

 increased in every case. 



Again the ratio together and separate is : — 



KC1 

 NaCl' 



together 



1 



1-66' 



separate j|j. 



NaCl 

 NaN0 3 



> V 



1 

 1-444' 



1 



» 1-679* 



KN0 3 



KC1 ' 



}> 



1 

 2-36' 



1 



» 1-488' 



KNO3 





1 



1 



NaNO,' 



2-45' 



3-277* 



